Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry Final Semester 1 > Untitled Deck > Flashcards

Untitled Deck Flashcards

1
Q

How do atoms become ions?

A

Atoms become ions when they gain or lose electrons. Gaining electrons creates a negative charge (anion), and losing electrons creates a positive charge (cation).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is the difference between a Cation and an Anion?

A

A cation is a positively charged ion, and an anion is a negatively charged ion.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is a period in the periodic table?

A

A period is a horizontal row on the periodic table.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is fission and fusion?

A

Fission splits a larger atom into smaller atoms. Fusion combines smaller atoms to form a larger one.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

How does Schrödinger’s quantum model describe the atom?

A

Schrödinger’s model describes electrons as existing in probability clouds (orbitals) rather than fixed orbits, with wave-like properties.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the Rutherford model of the atom?

A

Rutherford’s model states that electrons surround the nucleus and revolve around it in circular paths (orbits).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are the four regions of the periodic table and their locations?

A

Region 1: Alkali/Alkaline Earth Metals (Groups 1-2, leftmost)
Region 2: Transition Metals (Groups 3-12, middle)
Region 3: Metalloids (diagonal line between metals and nonmetals)
Region 4: Nonmetals (rightmost)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Where are the largest elements found on the periodic table?

A

The largest elements are found in the bottom left corner of the periodic table.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How do valence electrons relate to group numbers?

A

The number of valence electrons equals the group number of the element.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the typical charge of elements in each group on the periodic table?

A

Alkali Metals: +1
Alkaline Earth Metals: +2
Transition Metals: Varies
Nonmetals (Group 15): -3
Nonmetals (Group 16): -2
Halogens: -1
Noble Gases: 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are the groups and families on the periodic table?

A

Groups 1-18 include alkali metals, alkaline earth metals, transition metals, metalloids, halogens, noble gases, and more.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the danger/penetrating ability of alpha particles?

A

Alpha particles have low penetrating ability and can be stopped by paper.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the danger/penetrating ability of gamma particles?

A

Gamma particles have high penetrating ability and can be stopped by lead.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is the danger/penetrating ability of beta particles?

A

Beta particles have medium penetrating ability and can be stopped by metal.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What does a gas particle picture look like?

A

Gas particles are spread out and move freely.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What does a liquid particle picture look like?

A

Liquid particles are close together but can move past each other.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What does a solid particle picture look like?

A

Solid particles are tightly packed and vibrate in place.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What quantity is represented by ‘Kilo’?

A

Kilo represents 1000.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What quantity is represented by ‘Centi’?

A

Centi represents 1/100.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What quantity is represented by ‘Milli’?

A

Milli represents 1/1000.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What quantity is represented by ‘Hecto’?

A

Hecto represents 100.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What quantity is represented by ‘Deka’?

A

Deka represents 10.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What quantity is represented by ‘Deci’?

A

Deci represents 1/10.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Define density.

A

Density is the measure of how tightly matter is packed together.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Define mass.

A

Mass is the amount of matter in an object.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Define volume.

A

Volume is the amount of space occupied by a sample of matter.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Define pressure.

A

Pressure is the force exerted per unit area.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What is the relationship between pressure and volume?

A

Pressure and volume have an inverse relationship: As pressure increases, volume decreases.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What is the relationship between temperature and volume?

A

Temperature and volume have a direct relationship: As temperature increases, volume increases.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is the relationship between particles and volume?

A

The number of particles and volume are directly related: More particles = more pressure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What is the relationship between temperature and pressure?

A

Temperature and pressure have a direct relationship: Higher temperature = higher pressure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

In which type of decay does the atomic number decrease by 2 and the mass number decrease by 4?

A

Alpha decay.

33
Q

What type of decay emits electrons?

A

Beta decay.

34
Q

What type of decay emits Helium?

A

Alpha decay.

35
Q

What type of decay is emitted without change?

A

Gamma decay.

36
Q

What causes pressure in a container?

A

Pressure is caused by the collision of gas particles with the walls of the container.

37
Q

How can the pressure inside a balloon (flexible container) be increased?

A

Decreasing the volume increases particle collisions, raising pressure.

38
Q

How can the pressure inside a metal can (rigid container) be increased?

A

Increasing the temperature makes particles move faster, leading to more collisions and higher pressure.

39
Q

How do you solve for the unknown metal using density?

A

Use the formula Density = Mass/Volume. Subtract the initial water volume in the cylinder from the final volume to find the volume of the unknown metal.

40
Q

How do you calculate volume?

A

Multiply the dimensions of the object (e.g., 6.5 cm x 8 cm x 5 cm) and convert units if necessary.

41
Q

How do you calculate slope on a graph?

A

Choose two points (x1, y1) and (x2, y2). Use the formula Slope = (y2 - y1) / (x2 - x1) to find the slope.

42
Q

How do you calculate the distance traveled using the slope of a line?

A

Multiply the slope by the time (in minutes) to calculate the distance traveled.

43
Q

How do you use a graph to compare the density of substances?

A

Choose two points on the graph (x, y) and (x, y). Use both points to describe the relationship, e.g., ‘For every 10 mL, you have 75 mL.’

44
Q

What is the identifier for alpha decay equations?

A

The identifier for alpha decay is He 2/4 (or 4/2 He).

45
Q

What is the identifier for beta decay equations?

A

The identifier for beta decay is 0/-1 e (electron).

46
Q

What is the identifier for gamma decay equations?

A

Gamma decay does not release particles and looks normal, e.g., 238/92 U.

47
Q

What is the alpha decay reaction equation?

A

The equation is X/YB → 4/2 He + (element’s mass - 4) / (atomic number - 2).

48
Q

What is the beta decay equation?

A

The equation is n → p + β - + Ve (with a line above Ve).

49
Q

How do valence electrons relate to the group number?

A

The number of valence electrons of an element is equal to its group number on the periodic table.

50
Q

What is the typical charge of an ion from each group/family on the periodic table?

A

Group 1: +1
Group 2: +2
Group 13: +3
Group 14: +4 (positive or negative)
Group 15: -3
Group 16: -2
Group 17: -1
Group 18: 0 (noble gases)

51
Q

Name the elements that would have similar properties to calcium and barium.

A

Magnesium (Mg), Strontium (Sr), and Radium (Ra) would have similar properties to calcium and barium as they are in the same group (alkaline earth metals).

52
Q

List the elements that are in the same period as sodium.

A

The elements in the same period as sodium (Period 3) are:
Sodium (Na)
Magnesium (Mg)
Aluminum (Al)
Silicon (Si)
Phosphorus (P)
Sulfur (S)
Chlorine (Cl)
Argon (Ar)

53
Q

Explain how the sodium atom becomes a sodium ion (what does it gain/lose and how much)?

A

A sodium atom loses one electron to become a sodium ion (Na⁺), resulting in a positive charge.

54
Q

Explain how the sulfur atom becomes a sulfur ion (what does it gain/lose and how much)?

A

A sulfur atom gains two electrons to become a sulfur ion (S²⁻), resulting in a negative charge.

55
Q

What is atomic number?

A

The atomic number is the number of protons in the nucleus of an atom, which determines the element’s identity.

56
Q

What is atomic mass?

A

Atomic mass is the weighted average mass of an atom of an element, based on the abundance of its isotopes.

57
Q

What is an isotope?

A

Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons, resulting in different atomic masses.

58
Q

What is the law of conservation of mass?

A

The law of conservation of mass states that mass cannot be created or destroyed in a chemical reaction; it is conserved.

59
Q

What is a chemical reaction?

A

A chemical reaction is a process in which one or more substances are converted into new substances with different properties.

60
Q

What is a covalent bond?

A

A covalent bond is a chemical bond formed when two atoms share electrons.

61
Q

What is an ionic bond?

A

An ionic bond is a chemical bond formed when one atom transfers electrons to another atom, resulting in the formation of oppositely charged ions.

62
Q

What is the law of definite proportions?

A

The law of definite proportions states that a given compound always contains the same elements in the same proportion by mass.

63
Q

What is the trend of charge on ions as you move across a period?

A

As you move across a period, elements on the left tend to form positive ions (cations) by losing electrons, while elements on the right tend to form negative ions (anions) by gaining electrons.

64
Q

How do you name ionic compounds?

A

To name ionic compounds:
Name the metal (cation) first.
Name the non-metal (anion) second, changing its ending to ‘-ide’ (e.g., chlorine → chloride).
If the metal has more than one possible charge (transition metals), include the charge in Roman numerals in parentheses.

65
Q

How do you write the formula for ionic compounds?

A

To write the formula for ionic compounds:
Write the symbols for the cation and anion.
Balance the charges so that the total charge is zero by adjusting the subscripts.
If necessary, use the least common multiple of charges to balance them.

66
Q

How do you name covalent compounds?

A

To name covalent compounds:
Name the first element using its full name.
Name the second element by changing its ending to ‘-ide.’
Use prefixes (mono-, di-, tri-, etc.) to indicate the number of atoms of each element (except for mono- with the first element).

67
Q

How do you write the formula for covalent compounds?

A

To write the formula for covalent compounds:
Use the prefixes in the name to determine the number of atoms of each element.
Write the formula by placing the appropriate number of atoms for each element as a subscript.

68
Q

How do you name ionic compounds with transition metals?

A

For ionic compounds with transition metals:
Name the cation (transition metal) first.
Indicate the charge of the metal using Roman numerals in parentheses.
Name the anion second, changing its ending to ‘-ide.’

69
Q

How do you write formulas for ionic compounds with transition metals?

A

To write formulas for ionic compounds with transition metals:
Determine the charge of the metal from the Roman numeral.
Balance the total charge by adjusting the number of anions to cancel out the charge of the cation.

70
Q

What is the difference between ionic and covalent bonds?

A

Ionic bonds form between metals and non-metals, where electrons are transferred from the metal to the non-metal.
Covalent bonds form between non-metals, where electrons are shared between atoms.

71
Q

How do you name ionic compounds with polyatomic ions?

A

To name ionic compounds with polyatomic ions:
Name the cation (metal or ammonium ion).
Name the polyatomic ion, using its regular name (e.g., nitrate, sulfate).
If the metal has multiple charges, include its charge in Roman numerals.

72
Q

How do you write formulas for ionic compounds with polyatomic ions?

A

To write formulas for ionic compounds with polyatomic ions:
Use the charges of the cation and polyatomic ion to balance the overall charge.
Use parentheses if more than one polyatomic ion is needed, and place the subscript outside the parentheses.

73
Q

How do you name covalent compounds with multiple atoms?

A

When naming covalent compounds:
Use prefixes (mono-, di-, tri-, etc.) for each element to indicate the number of atoms.
The prefix ‘mono-‘ is not used for the first element, but it is used for the second element.

74
Q

How do you write formulas for covalent compounds from their names?

A

To write formulas for covalent compounds from their names:
Use the prefixes in the compound’s name to determine the number of atoms for each element.

75
Q

How do you name covalent compounds with multiple atoms?

A

When naming covalent compounds: Use prefixes (mono-, di-, tri-, etc.) for each element to indicate the number of atoms. The prefix ‘mono-‘ is not used for the first element, but it is used for the second element.

76
Q

How do you write formulas for covalent compounds from their names?

A

To write formulas for covalent compounds from their names: Use the prefixes in the compound’s name to determine the number of atoms for each element. Write the number of atoms as subscripts next to the element symbols.

77
Q

What is the naming rule for ionic compounds with group 1 and group 2 metals?

A

For group 1 and group 2 metals (which have only one charge): Name the metal (cation) first. Name the non-metal (anion) second, changing its ending to ‘-ide.’

78
Q

How do you name ionic compounds with polyatomic anions?

A

When naming ionic compounds with polyatomic anions: Name the cation first. Use the regular name for the polyatomic anion (e.g., sulfate, carbonate).

Chemistry Final Semester 1 (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions